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Question 21 1 pt: What is the reduction potential for the half-reaction AP*(aq) + 32Al(s) at...
What is the reduction potential for the half-reaction AP(aq) + 36 Al(s) at 25°C if [A13+1 -0.18 M and E--1.66 V? a) -1.84 V Ob) -1.67 V OC) -1.65 V od) -1.72 V e) -1.66 V
10. You want to know the standard reduction potential for the Cr* (aq)|Cr(s) half- reaction Cr3 + (aq) + 3e-→ Cr(s) y, your textbook only lists the following data for chromium: Cr3+ (aq) + e-→ Cr2+ (aq) Cr2+ (aq) + 2e-→ Cr(s) E' =-0.424 V E' =-0.900 V What is the standard reduction potential for the Cr (a)Cr(s) half-reaction at 25 °C? A)-0.741 V B)-1.324 V C) 0.382V D)-0.141 V E) 0.476 V
what is the reduction potential for the half reaction AL3+(aq)+3e-+AL(s) at 25C if AL3+=0.18M and E=-1.66v
For the cell shown, the measured cell potential, Ecell, is -0.3629 V at 25 °C. Pt(s) | H,(g, 0.707 atm) | H+ (aq, ? M) || Cd2+ (aq, 1.00 M)| Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, Eº, are 2 H+ (aq) + 2e - H (9) E° = 0.00 V Cd2+ (aq) + 2e — Cd(s) E' = -0.403 V Calculate the H+ concentration. M = 0.031 Incorrect
For the cell shown, the measured cell potential, Ecell, is -0.3709 V at 25 °C. Pt(s) | H,(g, 0.877 atm) | H+ (aq,? M) || Cd2+ (aq, 1.00 M) Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, Eº, are 2 H+ (aq) + 2e H (9) E' = 0.00 V Cd2+ (aq) + 2e - Cd(s) E' = -0.403 V Calculate the H concentration. [HT] = M
For the cell shown, the measured cell potential, Ecell, is -0.3687 V at 25 °C. Pt(s) | H, (8,0.873 atm) | H+ (aq, ? M) || Cd2+ (aq, 1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, Eº, are 2 H+ (aq) + 2e → H, (g) E° = 0.00 v Cd2+ (aq) + 2e- Cd(s) E° = -0.403 V Calculate the H+ concentration. [H+) = .0588 M Incorrect
Question 19 (1 point) What is AG°273 of the reaction 12(s) + Br"(aq) -- 21" (aq) + Br2() at 0°C? Br2 (1) + 2e - 2Br (aq) E half = 1.07 V 12 (s) + 2e - 21 (aq) E half = 0.53 V -1.0 * 105 J/mol 1.0 * 105 J/mol 5.0 x 104 J/mol 0.5.0 × 104 /mol
For the cell shown, the measured cell potential, Ecell, is -0.3711 V at 25 °C Pt(s) H2(g, 0.865 atm) | Ht (aq,? M) || Cd2+ (aq, 1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, E°, are 2 H"(aq) + 2е — H2(g) Eo = 0.00 V Cd2+(aq)2 e - Cd(s) Eo =-0.403 V Calculate the Ht concentration М
For the cell shown, the measured cell potential, Ecell, is -0.3707 V at 25°C. Pt(s) H(8, 0.857 atm) H+ (aq.? M) || Cd2+ (aq, 1.00 M) | Cd() The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, Eº, are 2 H+ (aq) + 2e- H,(g) E° = 0.00 V Ca2+ (aq) + 2e Cd(s) E = -0.403 V Calculate the H* concentration.
For the cell shown, the measured cell potential, Ecell, is -0.3689 V at 25 °C. Pt(s)H,(g, 0.789 atm) | H(aq, ?M) || Cd²+ (aq, 1.00 M) Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, Eº, are 2 H+ (aq) + 24 H, (g) E° = 0.00 V Cd²+ (aq) + 2e - Cd(s) E = -0.403 V Calculate the H+ concentration. [H+] =